Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -133.9 50.6 -285.8 S°(J/mol∙K) 266.9 121.2 191.6 70.0

asked by @lynsaed2 • over 1 year ago • Chemistry • 5 pts

I can't seem to figure this one out. I tried only taking into account gas states. Not sure where I am going wrong. I solved for delta H and S then plugged into the equation delta G= delta H-(T)(delta S)

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Hey again! So for this one notice how they only gave you 3 enthalpies of formation, thats because for N2 there isn't one since its in its natural state and the delta H f for it will be zero. So when calculating enthalpy of reaction use all 3 delta H f given but ignore N2 gas. For entropy you would use all 4. Temperature would be 25 deg Celsius again since we are at standard conditions. Everything else is the same like the last problem. Let us know if you are still stuck.

answered by @dashab2 • over 1 year ago
  • Will do, thanks Lynsae commented over 1 year ago